Method of converting the energy of fuel into electrical energy.



H. JONE.

PATENTED JULY 12, 1904.

METHOD OP CONVERTING THE ENERGY 0F FUEL INTOELECTRICAL ENERGY.

APPLICATION FILED NOV. 7. 1901.

N0 MODEL.

Hill!" ..i Ll;

No. 764,595, PTENTED JULY 12, A1904.

' EJONE. s METHOD 0E EONVEETING TEE ENERGY 0E EUEL INT0 ELECTRICAL ENERGY5 APPLIOATIOH FILED HOVHT; 1901.

2 SHEETS-SHEET 2.

N0 MODEL.

UNITED STATES Patntedfruiy 12,1904.

SPECIFICATION forming part of Letters Patent No. 764,595, datesJury'1' 2, 1s 'o4.A

Application filed November 7, 1901.

T0 all whom it may concern:

Beit known that I, HUGO J ONE, a citizen of the United States, residing in Chicago, in the county of Cook and State of Illinois, have in vented a new and useful Improvement in Methods'of Converting the Energy of Fuel into Electrical Energy, of which the following is a specification. f

This invention relates to methods of con verting the energy of fuel into electrical energy. The object of this invention is to obtain electrical energy from fuel by means of la gallvanic cell.

ble substance which is capable of. reducingv the oxid of some such metal as tinto the metal when heated with'it, therefore particularly the several kinds of carbon-, pure and impure, the carbon compoundswhichare ca pable ofeifecting that reduction,andanygas fuel byheating it with steam, as in thel manufactureof water-gas or with 'carbon dioxid or some similar substance; In any case the substance from which the electrical energy isgenerated is either the fuel' itself or a 'substance reduced by the fuel.:

' In that form-of the invention. whichfwill be used as ain-illustration .of the 'invention herefinafter 'the electric 'current v'is generated. by

'the action Y of .caustic potash upon. metallic tin, mercuric oxid vbeing used as depolarizeri` The' celljish'eated. Stannite'of` potassium is .watery solution.

- heatedwth coal orv carbon monoxid and the .l tinvreduced in'a furnacel according to methods .i similar-to those used ordinarily in the reducvtion of tinstone, except that the hot 'gilsesis- `s uiigig Afrom,thefurnace are -used'to heat the l cellv-'or va battery of several' cells'. There-.i

duced tin is aga-in used inthe cell'for the gen1-' ox'idis reduced'to mercurous oxid bythe 'acation'oft'he een. This mei-treue Oxide ree' mercuric oxid, which isagain 'used in this cell tion.

ated ,in thisprocess -is also used for heating xrous oxid'is4 oxidized-dischargetheir hot gases through' a passage-way below the cells, v .thusheatinggthe cells.l l which may be obtained from solid' or liquid samecn line A Aof Fig. l?. Fig. 3 lisatop plan View of th'e'furnace with the retort in -which the mercurous oxid is oxidized com-l 'Fig 5 vis a vertical's'eo'tiom partly in elevation,

Serial No. 815391. (No model.)

moved and converted intomercuric nitrate'by treatment with concentrated hot nitric acid, rIhe nitrate is broken `up by heat, yielding as depolarize'r` and lower 'oxid's ofnitrogen, from whlch nit'r1c acid 1s recovered by oxld'a# The' heat-of the furnace-gases generthe cells, likethat of. the gases 'of the red-uction-furnace. 'The apparatus in which these processes are carried out consists substantially cfg-a battery of galvanic cells,- a furnace for the reduction of the stannite, preferably a re verberatory' furnace, and a retort suspended 'wlthin a furnace'for the oxidationof mercu- 65 rous OXid to mercurio Oxid connected with a condenser-coil for' thereco'very o'f the nitric acid.' Both' furnacesfthe reduction-furnace andthatwith the retort in which the mercuan illustrative form'of the apparatus.

Referring 'to' -the drawings and tothe various views and reference-signs' 'appearing thereomFg'ure l is a top' plan view; of one of the'eells'.. Fig. 2 `is a verticalsection offthe In theaccompanying drawings I have shown bined with the condenser-'coil for the recovery l of thenitrie acid.A Fig. LLis a verticalsection j ofthe same.' apparatus, partly in elevation.' 85 o ffzthe entire plan,' c om prisi1`1g both' 'furnaces I' -The galvanicncellS-t'lfoneof which sof.'

9 0 partwherever occurs. 11nl thel several.l

" oiiid and -the mcrcurous oxid 17,ft 'orme '(il fr onif s it by deoxidation, so that they. e'annob'entertheg space lbelow, \Vhieh`=' is 3 ,the riode-space; ,-f-fthe same time this vessel'' il'poioi 1siearbongfv Serves. as the negative-plata. Vessel9'is`rn'ade1 lof some 'material that is che-1nically unaifected f by caustic fpotash.v u Resting upon vthe'bottoni' this` -ve'sseland in rnetallicfconta'ctl there? ed by?causticfallialies, alkaline lcarbo'n ates,

4and fby 'molten metallic@tink- The ,flat lpa'n- "fscrvesas areceptacle for-the tin, veithersolid 'fis.generated. "l`he tin is.in' electric contactA with .wire 28'tlnfoughclamp24, .the metal ot" f thelvessel 9,` and thei'i-on plate 16.`l .The nega.-

i `tiveiplate 10 is in. electric..contactjwithwire' A29 throi-igh clamp' 23.' Pipe 30 serves to supplythe tin to be oxidized in the molten con- 10 orplate 16, )sof that apart ofvessel 9 re-` dition; .Vessel 9 is larger than either vessel 'i mains unoccupied .by both vessel l'Qand plate y 16. r 4This part of if'essel 9 isipartiti'oned oli' by i -l'i'iaieapd Sliding door- 111,1 b0u1pf1whih objectsarehdd in'place b ya'ng'le 18, of'suitable -material. 1 late12 ismade ofaporous sub- #stance which'isnot'alectedby-causticalkalies "oralkaline carbonates'and.whichis not apt to 'cause-' local actionrby, aetingasan electrode.

lt maybef'madel of'sultid A'ot-calcium. In that s ectionot'vessel9 which is thus'partitioned off Fa porous. vessel21is'placedg This vessel is preferably squareins iape,isof as' .t o lit into the 'sectionL 'Itmay beprovided with handle-holes 19 serves to supply watery solution of barium hydro'Xid."f The solution." is preferably hot and saturated. I 'of 'vessel'QlL is'fstanni'te fof barium, obtained by precipitation'ofstannite of potassium by "the-'barium hydroX-ijdf-supplied by pipe 19. *The'uid 18,:showninfboth sections of vesfsel-9. and in vessel-1:10,' is a concentrated wa- 22, -softhat it can be lifted rup easily. Pipe The'powder- 2O at the bottom ery solution'lof "causticA potash. This solu- ;ti on.i's 'coveredbyajlayer of paraiiin 32 to .jp'reventabsor-ption`of carbon dioxid and of oxygen. from, the air.

Vessel 9 is protected against. loss o f mu'chfheat .by being covered on thefsiol'esv and c )njto'pfby thick sheets of as- :bestes 27 v2 6 25..'-f1'A-vstrip of electric insulating material 31, suchA as asbestos or marble, is 1placed below'the flanges of thecarbon vesel 10,'whereit restsonvessel 9. The electric currenti's obtained between wires 29 and 28. .60.'

.' .the battery is heated to a temperature somef lo'start the 'generation of electrical energy,

l fwhatfbelow the boiling-pointof the alkali ',.s'olu'tionL l The caustic potash and the mercu-` Iwithfproduction o'f. an electric current, the f oxygen 'beingv su p'plied'by the niercuric oxid, v whicliis'thereby reduced to .mercurous oXid, or',"'i-f there is insuliicient supply of it, tome- -tallic-mercury, as follows:

of the following two reactions if the fact is ignored .that the hydrogen ,is oxidized in vthe nascentstate andv notl liberated as such if there is proper lelectrolytic action:

.-jsfi+KoH+H'ZofsosLKoHJfaH f ,Q'Hfngortoafngo In-lease of? insufficient supply of `mercurio oxidft'he -lastfreaction may be modilied as fol- Thcstannous oxid formed in the battery reaction is gradually dissolved as stannite of potassium, thus:

The stannite of potassium diffuses through the'solution and passes through plate 12, the pores of which are wide enough to let it pass readily into the porous vessel 21, the sliding door 1l being raised all the time except immediately before and after the addition of barium-hydroXid solution through pipe 19, when it is closed to prevent the suspended sediment of barium stannite from passing into the anode-space and covering the surface of the tin. Inv the porous vessel 21 the stannite of potassium is precipitated from time to time, so as to prevent the liquid from becoming saturated with it, the preeipitant being a hot concentrated watery solution of bariumhydroxid, which is introduced through pipe 19. The reaction is as follows:

The barium stannite is allowed to accumulate and is then removed by raising the porous vessel 2l out of the liquidl8 and emptying it. This barium stannite is reserved for re` duction to metallic tin, which is then again supplied to the cell ffor the production oi' electrical energy.

1t will be noticed that the removal of the battery prod uct-the stannous oxid contained in the potassiurnstannite- -prevents theaction of the battery from being stopped by saturation of the electrolyte with stannous ox'id coupled with accumulation of undissolved stannous oxid on the surface of the metallic tin. Furthermore, the precipitation of the battery/"product permits of a continued pro-v duction ot electrical energy and! of a continued supply of metallic tin for the battery voiiid act on the metallic tin, oxidizing it reaction. The tin may be supplied through This-reaction may be considered as consisting v with is an iron 'plate-16,provid`ed witha ledgev I15, running lalong its edge 'and' constituting,"

with the plate, ailat pan; The ledg'e ismadev [f ofsome material whichis chemically unailectf- I IOC IIO

pipe 30 in thevmelted condition. The electromotive force of acellof this kind is 1.03l

volts. The current strength of-a kcell of the described form and of the capacity of oney gallon of liquid is twelve amperes when the external resistance is .O4 ohm.

The mercurous oxid obtained by-the batteryreaction in vessel 10 is'allowed to Az ic'cu- Jrnulate until nearly the -whole of the mercuric oxid is converted into mercurous oxid. vThen the mixture of the two oxids is removed by suitable means and a suitable quantity of mercuric oxid put in its place.

holes in suitable positions 45. Within the powders 35. The upper part is provided with a screw-cap 37 and a pipe 39 suitable for the introduction of steam into the retort and provided with a valve and communicates with condenser-coil 41 through pipe 40. The upper part of the retort 34 can be detached by means of Hanges 38, so as to affordl access to the lower part of the retort 36. Condensercoil 41 is cooled ,by cold water contained in condenser 43. Pipe 42 serves to convey any liquid that may form by condensation of 'vapor in condenser-coil 41 to vessel 44.

The mixture 35 of mercurous and mercuric oxids is placed into the lower part of the retort 36, the upper part 34 having been detached.

, furnace 33 and the retort heated.

Concentrated nitric acid is then added to the powder in quantity suiiicientto convert it vlnto mercuric nitrate and is mixed with it.

Then the upper part of the retortv 34 is replaced' and connected. A fire is started in the The mercurous and mercuric oxids are thus converted into mercuric nitrate,the reactions being as folows:

sufiicient for the reaction, an additional quantity is added through screw-capV 37. Steam is admitted through pipe 39 and the heating of the retort continued.. The heat breaks up the mercuric nitrate as follows:

Hg(NO3)2= HgO-l-QNOz-l- O. Theimercuric oxid is thus obtained as desired.

.Thepitrogen peroxid thus evolved inthis and in the second preceding reaction is mixed with the'steaia,`is carriedinto the condenser-coil 41, mixes there with air entering through the open The appara-- tus in which mercuric oxid is recovered from the mercurous oxid by oxidation is shown@ in Figs. 3 and 4. This apparatus comprises a furnace 33, provided with one or two draftl topof the coil, and is thereby oxidized to nitric lacid yas follows: l `ano;+H2o'zito54n2o'4iso: 1

. v v QHNOa-l-NO l NO-l-JQvzvNOz.

The nitric acidl condense's, Hows into vessel .44

throughp'ipel42 'and-may' again be usedfor p It will noticed thatthe oxygen for'the'oxi- `dation of thel mercurous oxid isultimately 'taken from theair, the nitric acid being recovered. 'l i 'v x An additional advantage is secured in operating cells the kind-described if these'cells can be combined Withan'apparatzus vfor the recovery of mercuric oxidfrom mercu rous oxid'.

'The hot gases issuing from the furnace.,l the .heat-ofwhich"would-otherwise be lost, may i'be ufsed k'to 'keep the cells at an elevated tenn-4 Furthermore, a furnace is used toreduce the barium stannite whichis obtained from the cells, as described hereinabove, to metallic tin, by means of coal or some other .suitablev fuel, the tinv to be used again in the cells for the production of electrical energy. 1f this furnace is combined in the same plan with the cells, the hot gases of this furnace may also be utilized by applying them to the cells for the purpose of keeping them hot. A plant in which the hot gases of both furnaces are thus utilized isshown in Figs. v5 and 6. For the reduction of the stanniteofbarium a reverberatory furnace 47 may be used. This furnace does not differ essentially from other reverberatory furnaces used for, the reduction of tin ores, except that one of the receptacles voxidation of m'ercurous oxid to mercuric oxid.

IOO

door substituted for it, so that the charge on the hearth 48 may be worked from both sides through the doors 57 instead of being worked through a door opposite the fire, this latter door '50 being converted into a closed flue in this-case. @Through this flue 50 the hot gases of thevvfurnace 57, which would otherwise` be wasted, pass into the passage-way 51 below the cells 9. The cells, which are separated by sheets or' asbestos or other insulatingl material for `electricity and which may be connected in series in the ordinary manner, are thus heated by the gases, which subsequently are discharged into the air through the smokestack 54, which causes them to move. AThe passage-way grows wider where itisnearer the smoke-stack, so as to distribute the' heat uniformly bysecuring a larger surface ofcoutact with the less-hot gases. .Injthe same manner the hot gases from the oxidation-furnace. 33 are drawn through the passage-Way 51, eX-

cept that they may be allowed to pass through pipe 46 and thereduction-furnace 47. Pipe 46 is provided With a branch pipe 53, through which air may be supplied to furnace 47 yif that coming from furnace 33 alongy with the y11s e hot gases is not sui'cient. vBoth pipes i6 and i 53 are covered with asbestos to reduce the loss of heat, and each is provided with a valve 55 and 56, which serve to regulate the draft. As the lhot gases coming from furnace 33 contain carbon dioxid, which is reduced to carbon monoxid to 'some extent when it strikes the hot coal in furnace 47,- the arrangement promotes the reduction of the tin compound, since it is the carbon monoXid that reduces it. The

reductions of the carbon dioXid by carbon and, of barium stannite by carbon monoxid are as follows:

coilfczeco BaSnOz-l-CO: 002+ Sud-Ba@- Thev barium oxid thus obtained is dissolved in hot water and again used for the precipitation of stannous oXid in vessel 21, while the tin is introduced into the cells for further generation of electrical energy, as already stated.

' The battery may be operated at a tempera- A ture considerably below 300" centigrade.

' temperature above 800'"centigrade is notindispc'nsablev The temperature may be as low as 150Q centigrade; In this case the tin forming the positive plate evidently ,solidies rihe solid state ofthe tin', however, does not, or

- action.

not materially, interfere .with the battery re- This lowerlng o temperature is understood to be accompanied by a corresponding lowering of the boiling-point of theel-haii. solution.

: itannic oxid, or stannate of potassium is not formed inthe electrolytic oxidation of thetin, i

ory at least tea i-'ery. limited extent, provided the oxygen of the air is excluded and the cells are kept at-fa constant elevated temperature. lf

the cells Were allowed to cool. the potassium ',Stannite in solution would be liable to formA stannate according 'to the following reaction:

vrlhus by keeping out the oxygen of the air and by maintaining a constant elevated temperature the necessity of reducing stannic compounds, which, as is known, would require a higherl temperature for reduction than the stannous compound, is obviated.

The apparatus need, not be made exactly as described. Changes niet" be made which do l l not materially afiect tiza chemical reactions or Erbe production of electrical energy. rlhe numricerca are capable of acting as acids toward alkali and which are readily reduced by carbon with formation of carbon dioXid also produce electric currents, lwith alkali as the electrolyte and mercurio oxid or a similar metallic-oxid as the depolarizer. The lead can be recovered as barium plumbite by precipitation with lbarium hydroxid similar to the tin and the barium plumbite reduced in the same manner as the barium stannite. Cadmium may also be used in placeof tin, although its oXid has no acid properties'. Barium hydroxid is not the only substance which can be employed for the precipitation ofthe stannous oxid. Other bases, especially the hydroxids of the other alkali-earth metals, may be used. The

barium hydroxid, however, is preferred, be

cause it is more soluble in water, particularly in hot water, so that the addition of much water is avoided. i

One of the essential features which distinguishes this invention from-old devicesl con- Sider to be the combination of an easily-reducibi'e metal, as the positive plate, with an alkaline electrolyte. 'lvhose cells with alka# line electrolyte in which zinc is used as the posit-ive plate would Vz inswer the purpose of i'ircilucing electrical energy from fuel, but impei-fe` *l since the reduction of oXid of zinc tained m-fv-educticn romcthe oXid-by means fel , i consumed-in the reduction,v ni it cbtained from tin-steric by the same process represents about twenty per cent. of the energy of the coal, andstill more when it isobtainedfrom freshly-precipitated 'ents only abo'nt2.5 per, cent. of

vin very i isteuL `lli/*bile metallic zinc obstaniim-lsi oxi'd, theistann'ousoxid bein g" reduced 'more readily and at a lower temperature than` v the lstannic oxid and particularly so if it is formed by recent oxidation in presence of Water instead of being a hard natural mineral. i

IOS

As the tem per'ature required for the reduction `of the loweroxid of tin is but little more than half as high as the* temperature required for that of the higher oxid, taking the temperature of the surroundings as zero, the fall of heat toward the surroundings, and consequently the loss of heat, is onlyabout half as high with the lower oXid, Therapidi'ty with which freshlyformed andv iinely-divided stannous cxid reacts accounts for a further decrease of the loss of heat, the time required for reduction and during which ahigh temperature has tc be maintained being reduced to about one-half. rldhe great diference in the efciency et ore reduction and ef that of freshly-formed metallic, oxide dees not to have been taken in'ic accounthiiertc by inventcrs trying tc ccnvert the energy of ccal inte ei-ectrical energy by means ci gaivanic ceii4 ie iov.' ing-point ci" tin evidently else faciiitates the reducticn.

The difference the yieid reducticn of zinc and of tin is to a large extent accounted for by the -fact that zinc oxid does not form carbon djoxid when heated with carbon, but

carbon lmonoxid, .which escapes unused, and,

furthermore, by the necessity of maintaining a` very high .temperature for a considerable time in the reduction of this oxid.

Owing to the difference in the yield,vit is,`

I should think, an important advantage to' be able to use for the generation of electrical energy tin or some other easily-reducible metal linstead of zinc, particularly so when the advantages of an alkaline electrolyte can be comfis bined with the advantage of an easy reduction. One of the advantages of an alkaline electrolyte is thefact that the metal which is dissolved by it vforms an oxid which is more readily reducible than the alkali, itself, so thatthevreduction of the solvent is obviated in the subsequent reduction of the battery product.

. VAn example will illustrate this advantage: If metallic zinc is dissolved in sulfuric acid, the

regeneration of the metallic zinc from the sulfate of zinc formed by reduction withlcarbon will, if the common method of reduction is' employed, involve the reduction of the acid radical S03 contained in the sulfate to reduction products which isobviated bythe SO2; This will be doing useless work unless the oxidation energy is utilized besides that of the metallic zinc obtained in the reduction'. It is this necessity of utilizing two or more I employment of an alkaline liquid. Ifmetallic zinc is dissolved in caustic potash, there-` sulting Zincate of'potas'h can evidently be re- .duced to metallic zinc without a simultaneous reduction of the potassium oxid'containedinv the zincate. The advantage is securedby the fact that the zinc is dissolved in a solution of lthe oxid of a metal which, unlike the 'acidy radical SOS, is able to withstandthe reducing action of coal or of fuel-gases at a temperature atwhich' -the' ox id of the-zinc is reduced;

The advantage, then, which I secure by dis-' exclusively, thermocu'rrenta.A `This seems toI I solving tin or anyother metal in alkalifor in some other oxid which is morejstable than the oxid oftin formed inthe dissolution is they f factthatI have only the oxid of tin to .re--

duceand 'not' the oxid of any other element.

Besides, the reduction of barium stannite jis equivalent Vin thatfrespect to that of potassium lyte makespossible true electrolytic action of a chemical nature. while those currents 'produced without such a solventare mostly, if not be due to the fact that electrolytic dissociation takes placeonly insolution. -I Afound thatf. certain galvanic cells which do not produce a current without water are capable of vproduc'- v The presence of ing one upon addition of water to the electro-vv lyte. It is-therefore very desirableto retain the Water in the electrolyte whenever al cell is heated, since vneither a high current strengthy nor a high yield is to be expected from a current of exclusively thermal origin. Caustic potash is an ideal substance forretaining` Water in electrolytes, since its avidity for water' isgreat andthe boiling-points of its 'watery solutions exceedingly high; Caustic soda answers the purpose almost but not quite as well, Since theboiling-points of its watery solutions of definite concentration are lower than those 'of potash solutions. Although' it'is possible to produce an elec.-

as electrolyte Without having anything but thev oxidof the dissolved metal to reduce, the

current obtained in this 4manner is much weakerthan that obtained With caustic alkali;`

8o tric current'with certain neutral salt solutions as electrolyte, owing to the corrosive -action of the alkali, whichv makes the battery reaction energetic. vThe watery solutions of ammonium nitrate and sodium chlorid'are capable of acting as electrolytes with tin as the positive 'plate and mercurio oxid as the depolarizer. The currents produced by these combinations are much weaker than that produced l with caustic alkali as theelectrolyte. rI he alkali-then 'secures an energetic reaction. '.It 95 also secures a more'rapid solution of the me tallic-oxid formed. in the battery reaction.

Another circumstance'which makes the acl vtion of the cell described herein above ener'- getic is the fact that the oxid vof tin'possesses 'acid-properties'in a comparatively highv der l "grec, so 'that its energetic reaction with al' mais 'accounted for.` Thatmemuic an with which'v .canv be utilized for the production of Ishouldithink,1attributable to those propervhot concentrated alkali vgenerates hydrogen .Is- .electrical energy, asin the cell described, is, v

ties of both-substances' which are conducive Y tothis effect and not merely to the properties; 1 .ofone of these substances. 4

Ho Analkalineelectrolyte affords considerable n 1 convenience and saving of expense inthel building and 'preservation of cel1s since the vcells may be made of. some ,suchV cheap durable material as iron, while itis difficult to find a ed by those acids which possess enoughfavidityfor the production'of strong electric cur-v rents-- Another disadvantage connectedlwith the use of acids and eliminated; with that ofi an alkali is, .asis-known,v the eva oration of the suitable substance which is entirely unaiectacidl and .contamination of t 4e airV withv its vapor, particularly at lan velevated temperature. I also secure by the use of an alkaline electro-' v iyte .those 'advantages which analkaline elecrtolyteaiords in other cells-.for instance, in 4 'theEdison-Laliandecell. The'internalresistf ance-is comparatively low, although this is -partlydue tothe elevated temperature, since the resistance ofV electrolytesv decr'eas'es'with any, of thatloc-al action which would result 1t metalsother-'t'lian tin andv soluble in alkali wl'ierepresent and in contact-With thetin. The

' presence of such metals canevident'ly beeasily avoided by using tin free. from'other metals,

" and even ifany metals should accidentally contaminate the tin those which are not or but slightly soluble in alkali Will evidently again be separated from the tin when it dissolves in the'alkali. purify itself to a certain extent. Before any metal Acan permanent-ly contaminate the tin it must not only be soluble in alkali, but must evident-,l valso be precipitated by barium hydrate,

it must have a low melting-point and be rey*duce-d bycarbon inonoxid, Otherwise it'w-ill evidently remain 1n solution when the tin is precipitated or remain solid when the, tin

meltsl or remain in the .oxidized form whenl the tin is reduced. rfhe use of an alkali o r an `alkaline earth evidently helps in effecting the separations of other metals from the tin in at least two instances-namely, in the solution `and theprecipitation of the metal. This' self-puriiication of the tin is undoubtedly responsible to a certain extent forthe high efieiency of the cell.

be too great to be accounted formerely by the keeping out ot' foreign metals.

'Ihe only cell which Iknow to have any essential resemblance with the cell covered by thlils application 'is that known as Borchers ce rent can be produced from carbon monoxid if alkali is substituted for the acid electrolyte, so far at least'as I am able to see, -for the reason that copper compounds' in alkaline solution do `not 'seem to be reducible by carbon monoxid at the ordinary temperature.

` The effective or useful combination, then, of an. easily-reducible metal with an yalkaline electrolyte seems to be new. v

It has been asserted that no electric current at all is. obtainable. from carbon monoxidin Borches cell even in acid solution, and this. is ascribed to the ineiiciency of atmospheric oxygen as depolarizer. It seems, indeed, that free oxygen does not aid in the production of a current, or not much unless it is previously combined with another substance or at least absorbed by some such .substance as spongy platinum. It will bev noticed that in accord- The tin therefore may be saidto I have shown that theuse of an alkali as electrolyte besides the ele` In this cell, however, no electric 'cur` lance with these circumstances I combine the I oxygen of the air with -m'ercurous oxid Afor the purpose of depolarization'.l Besides be;-

- ing an e'ective depolarizer-themercuricoxid,f

as well as other metallic oxids which'mayf be' i I -used as depolarizers, offers the advantages ofremaining undecomposedby the alkaliand of being easily regenerated. afterfdeoxidation I and without the consumption of any substance beyond atmospheric oxygen and .fuelr Furthermore, it causes but littlewaste ofvenergy when acting asadepolarizer. 'In the Edison- Lalandecell a considerablepartof theoxidation energy or'. the zinc is Wasted in breaking V up the cupric oXid used as depolariz'er." -As the energy required to reduce mercuricjoxid.

to mercurous'oxid is only about half as much as in the case of cupric oxid for the same amount ing-otl energy by the use of mercurio oxid-as described. Y

Tothe energetic-oxidizing actionof the mercuric oxid when actiiigon metals like tin of oxygen given o, 1 eliect considerable savj or antimony I attribute thefact thatI obtain with a comparatively feeblefeleetropositive metal, such as tin, that the battery reaction proceeds rapidly, and that the current strength is comparatively high.

The -principal advantage of an elevated temperature is an accelerated battery reaction and anincreased current strength'owing to the increased tendency of the tin to be'oxidized in contact with alkali and tothe tend-v ency ofthe mercurio oxid to giveoif oxygen at an elevated temperature. By promoting the oxidation ofthe metalwhich is'but moderatelyelectropositive the elevated temperaturemakes possible a highyield.` In the cold 1 as high an electromotive force asl'volts IOO.

the tin would givebut a feeble current, if any 'at all', and the' more-strongly.-electropositive metal would have to be usedv in order. to obtain a strong current. tate a greater loss of heat `in the reduction of the metalliccompound formedfrom the metal, since stronglyfelectrppositive metals require comparatively'high temperatures for reduction. It is this loss which is largely avoided IOS This would necessiby'an elevated temperature.V At the same time the stannous oxid Vis dissolved more rapidly, so that the partial or complete stoppage of the current by an accumulation of the oxid on the surface of the tin is prevented and the dissolved stannous oxid can be precipitated more rapidly. These advantages may be se l cured without cost, since the hotfurnace-gases which heat vthe cells would-otherwise bel Wasted. The special advantage consists in that the cell may be stopped easily by simply-- lowering the temperature. The stoppage of the current may also be brought about by discontinuing the addition of the barium hydrate.

In this case the tin is gradually covered by-a film of oxid which retardsand finally almost festatiou of the strong afnityof-tin for'oxyffl reduce' the tendency of the tin to be oxidized,

' the cold and without thepresence of alkali, it

-acid evidently also proves that afnity to be'jaf.

.Strongfreducer' makes a'good posi-tiveplate ini a galvanic cell, and it is fortunate that A "can v yetv be reduced from itsy oxygenfcom# 35" plate, as is vindicated by its position inthe .reducible metal.

entirely stops thebattery reaction@ f IStillan-I.` other way of stopping thiscell isbyjdisco'nf tinuing the supply oftin.l .l The use of tin as fthe. positive plate offers'- several advantages. Althoughthere are sevwhich therefore react with'. alkalhthe'fuse of x which as'electrolyte is very desirable for its action with alkalil and 'affords convenienfce'in that it can be 'supplied Ito the battervrinftheliquid state, its meltingepoirit being' low 7' 'Tlle fact .that its reaction with Ahot alkali' i s `acconifpan'ied by formation of hydrogen seemsftoyaecount largely for 'thest'rong elect ric i curient. it produces in the'cel'l; Ibeliev'e", i n` d eed,-thata large part of the-current'is. due to' the elec? trolytic oxidation .of A the nascent 'hydrogen Considering, fu'rthermore, the fact .thatiztiri reduces mercuric oXid Aunder water,v even'in is not surprisingthat the electrolytic oxida- -tion of tin by mercuric oxid in this cell is. vio. lent. This reaction, as Well `as' the-.formation of hydrogen, isA evidently not the -only-rnani-'- gen. The violent oxidation-of .tin-byjnitricf strong one. It is not surprising-'that .such- 'a the tin pounds with comparative easel in spite 'of-Hits' strong ailnity for oxygen. Furthermore,it -is capable of producing a comparatively high electromotiveforce when used as the positive electric tension series of metals, in spite of the fact that it is but a feebly basic and easily,

The difference of the temperatures at which tin decomposes Water and at which its oXid is reduced to the metal is not as great' as with most other. metals. This is another reason Why tin is preferred. If some such metal as zinc were to be reduced, the reduction plant would evidently have to be at a very high temperature, while the batterywould not need to be'heated at all.v Y The hot furnace gases would'be useless, and the vhigh' temperature of the reduction plant would naturally cause considerable loss ofheat, while vin the case of tin the battery and the 'reduce tion plant may be kept at approximately the same temperature.

By precipitating the tin it is possible to obtain a comparatively strongcurrent, because the solution is not allowed to .become saturated With the tin. Such a saturation would and therefore Would also reducev the rate of production of electrical energy.`

Thecarbon cathode is an important means for the production of a strong current. It

.giv'e'sa-:much strongerjcurren'tjthanniost niet .Thisl attribute large-lv;

)on in theclcotrical ten- Q which fnlakejs itl possible vely'highelectromotive2 l l'thosefmetals'wliiehare .but1v si .t`1ve,jas the :positive plate." i anadvantage'this vis will be ..,@odfif.irisomkleed-r=- *l that'itis just-.the `feeblyelectopositive metalsA many advantages, thetin excels 'infrapid ref,

. i-'febly'lor'e .forins'tance, lead, antimonyf, andarsenicf-and:

; carbonaceousi fuel.' y 4.

'as and for-the purpose set forth'. I

Which-ia' ,ord afliig'h yieldi'njthe reduction.'

"s eful, and desire carbomas tlief positive 'pIate'Wtli lan valkali as and thenlr'educing that battery productivhich'.

energy of fuel, and repeating the .oxidation the metal withgeneration'of electricalener 2. The method;offgenerating electrical .en-

the o'xid vof-'xv'hic'l f ldsf-ichiefi y carbonjdioxid metal 11i its'riediiction'by 4fcell; generating electrical of the metal, and then" reducing 'that battery j' product 4Whicli contains'tlue nietal oxidized in 'the battery reactiomto the iiietalj-byvnieans energy 'byoxida'tion I of theoxidation energy o f fuehand repeating the oXidati'onof-the metal Vwith generation of electrical energygas and for tlie'purpose setr forth., Y'

The method j of generatingjelectrical eriergy which consists in first conibininga metal, the oxld of which yields chiefly Carbon dloxid in addition' tolthe metal s in its reduction .with

carbon,as the'positi'vepla'te withan alkali as the. electrolyte, and carbon, as the negative' plate, .in a galvanic-cell, generatingelectrical energy-byoxidation of the metal, and lthen' j ..115 the metal oxldlzcdin.thebattery reaction-,to .the metal Abyineansof-thejoxidation''energy 1 of fuel,'and lre'peatingthe oxidation of the metal with generation of. electrical energy,.as 'z 120 4. The method of generating electric-al enf 'A .e'rgy which consistsin first combining a metal v j the oxid of whichyields c'hiefly'carbon dioxidreducing that battery'piodu'ct wliiclr'contains and'for the purpose setyforth. l

in addition' t0 the metal -in its reduction with'. -I y carbon, as the. positive plate {with analkali as ofthe metal, and 'then reducing thatbatte'ry'- ..12 the electrolyte and 'a porous ycarbon .vessel as.

thc negative plate, serving-at the same tiniefas'xjv Aarece-ptacle for the'depolari'zenin'agalvanic 1',.

cell, generating electricalenergy by'oXidation T g roo- . 5. The method'.'ofv generating electrical encarbon, asfthel positive plate with an alkali as theelectrolyte vin a galvanic cell, generating .'hydrogeu-Withfth'at' solution of alkali las the i lib. OXid'ofwliich'yield's chiefly carbon dioxid an 'eley'jatedv temi'ieratureI and then reducing '.that battery productwhich'contains the metal oxidiZedinf-.t'he vbattery reaction to the metal f.' bymeansof lthe oxidation energy of fuel, and

repeating' the-oxidation of the metal with gen- '9-2 theelectrolyte infa'galyanic cell, generating" faction. andl Whichisin'a finely-divided state .to metal'by1-r`neansof the oxidation energy carbon, and Which-..iscapable,of 'forming a 55:2

" f whichtonainsae mantengan ma@ barea,

-v producty whichcontainsthe .metal oxidized in 'g'.'the battery react'ir'in'-, to the metal by means j :of y.the oxidation energy of fuel,A and repeating g' A.the 'oxidationgofthe metal with generation of electrical energy, as"and for the. purpose set ergy Whichconsists vin first combining a metal -in addition f t'ofthe metalin its reduction by electrical energy-by oxidation of themetal at eration .offelectrica'l energy, as and for the purpose set '0rth.` f .f 16,5 Theme thod o f'generati'ng electrical. energypwhichconsists-in first combining a metal, vthe oxid ojwhich yields chiely carbon dioxid inedditiontothel metal in its reduction by l'carbon, as -thefpsitive plate with an alkali as y. oxidation of the metal, ndthenzreducingthat battery product which .containsfthelimetal .oxidized inthe battery re of' uei',fa nd .repeating-the oxidation of the' tal-' -Withgeneration of electrical energy, as" ndfor-thepurpose set forth. ?.fflThemethodpf generating electrical en'; rgy which consists in' first combining a metal,

the-.Oxidfof'whieh yields-'chiefly carbondioxid i in addition to the "metal in its reduction by.l carbon, and which is capable of. generatingpositiye-'platef yvith van alkali as the. electrolyte ."inf a galvanic cell; generatingelectrical energy hatfbattery productjyvhich contains themetal j vxid ized iin' fthe". battery ,reactin, the metal neatine the foxidationofthe mtal with een* l. 1 asjandfurthe.

eration'j jf" ectrica rrrosesetfrt 5 d of .generating electrical enfe'rgy'wh i'chc'ons'ists i'n'r's't 'combining a metal, theoxid'oiwhichl yields. 'chiefiycarbon ldioxid n v addition to the. metal"` in its reduction by higher` and 'a loWer. oxid,- `as the positive'plajte withl an y alkali as the. 'electrolyte in a galvanicA feeli, .generating electricalene'rgy by oxidation' of thetal -andwithj formation of the coml'ence,l andxthenreducing that battery product l'tery' reaction 'to'jtli'ej'rnetal'by means f the.'

x'idation: energy'. of' fuel, 'and repeating the v byoxidation' ofthe r'netahlaiidv then reducing l electrical energy, las forth.

ergy'which consists in first combining a metal,

in addition to the metal in its reduction by carbon, as the positive plate with an alkali as the electrolyte in a galvanic cell, generating electrical energy by oxidation of the metal, and then reducing that battery product which contains the metal oxidized in the battery reaction to the metal by means-of c arbonaceous fuel as reducing agent, and repeating the `oxidation of the metal with generation of elec- 10. The method of generatingelectrical energy which consists in iirst combining a metal,

carbon, and is capable of acting as an acid toward alkali as the positive plate With'an alkali as the electrolyte in a galvanic cell, generating electrical energy by oxidation of the metal and then reducing that battery product which 'contains the metal oxidized inthe battery reaction, to the metal by means of the oxidation energy of carbonaceous fuel, and repeating the oxidationof the metal with generation of electrical energy, as and for the purpose' set 11. The method 'of generating electrical en tin as the positive plate, with an alkali as the electrolyte vin a galvanic cell, generating electrical energy by oxidation of the tin, land then 'reducing that battery product which contains taili'c tin by means of the oxidation energy of aca'rbonaceous fuel, and repeating the oxidaenergy, as and for the purpose set forth.

which consists in first combiningametal, tn e oxid of which yields chiefiycarbon dioxid theelectrolyte and a compound containing oxygen and-capable Ofgdeoxidation as'the dethe deoxidation of' thecoiznpound containing uct which contains the metal Aoxidized in the 1 the 4oxidation energy of carbonaceous fuel, and repeating the oxidation of the metal with the g eration of electrical energy, as'and for 'the purpose set forth. i 13.v The method of generating electrical energy which consists in iirst combining a metal, .the oxid of which yields chiefly carbon dioxid the electrolyte and a metallic exid' as the de- Athetin oxidized in thebattery reaction to me;y

vinY .addition to the metal in its red-uctionby carbon, as the positive plate with an alkaline and for-the purpose set 9. The method of generating electrical enthe oxid of which yields chiey carbon dioxid trical energy, as and for the purpose set forth;

the oxid of which yields chiefly carbon dioxid in addition to the metal in its reduction by ergy which consists in first combining metallic f.

lool

`tion'cff. the tin with generation -oi' electrical I O5 l2. vThe method of generating electrical en-v 'inadditionto the metal in its reduction by carbon, as the posi-tive plate with an alkali as IIO 'polarize-r in a galvanic cell, generating-electrical energy by voxidation of the metal,` and r1 5 j oxygen, and then reducing that battery prod battery reaction, to the metal bymeans of l electrolyte in a galvanic cell, generating electrical energy by oxidation of the tin, precipitating the tin oxidized in the battery reaction and dissolved in the alkaline liquid by addition of the hydroxid of analkaline earth with formation of the stannite of that alkaline earth, and then reducing the stannite thus obtained to metallic tin by means of the oxidation energy oficarbonaceous fuel, and repeating the oxidation of the tin with generation of electrical energy, as and for the purpose set forth.

15. The method of generating electrical energy which consists in first combining metallic tin as the positive plate with an alkali as the electrolyte in a galvanic cell, generating electrical energy by oxidation of the tin, precipitating the tin oxidized in the battery reaction and dissolved in the alkaline liquid, by addition of the hyd roxid of barium with formation of the stannite of barium, and then reducing the stannite thus obtained to metallic tin by means of the oxidation venergy of carbonaceous fuel, and repeating the oxidation of the tin with generation of electrical energy, as and for the purpose set forth.

16. The method of generating electrical energy'which consists in first combining a metal, the oxid of Which yields chiefly carbon dioxid in addition to the metal in its reduction by carbon, as the positive plate withan alkali as the electrolyte in a galvanic cell, generating electrical energy by oxidation of the metal, and then reducing that battery product which contains the metal oxidized in the battery reaction to the metal by means of the oxidation energy of carbonaceous fuel in a furnace, heating the galvani-c cell by applying the Waste gases of the furnace to it, and repeating the oxidation of the metal with generation of electrical energy, as and for the purpose set forth.

HUGO J ON E. 

